Question

The electron in a hydrogen atom is excited to the n = 6 shell and emits electromagnetic radiation when returning to lower energy levels. Determine the number of spectral lines that could appear when this electron returns to the lower energy levels, as well as the wavelength range in nanometers.

Answer #1

An electron in an excited state
of a hydrogen atom emits two photons in succession, the first at
3037 nm and the second at 94.92 nm, to return to the ground state
(n=1). For a given transition, the wavelength of the emitted photon
corresponds to the difference in energy between the two energy
levels.
What were the principal quantum numbers of the initial and
intermediate excited states involved?

A hydrogen atom transitions from the n = 6 excited state to the
n = 3 excited state, emitting a photon.
a) What is the energy, in electron volts, of the electron in the
n = 6 state? How far from the nucleus is the electron?
b) What is the energy, in electron volts, of the photon emitted
by the hydrogen atom? What is the wavelength of this photon?
c) How many different possible photons could the n = 6...

1. a. A photon is absorbed by a hydrogen atom causing an
electron to become excited (nf = 6) from the ground state electron
configuration. What is the energy change of the electron associated
with this transition?
b. After some time in the excited state, the electron falls from
the n = 6 state back to its ground state. What is the change in
energy of the electron associated with this transition?
c. When the electron returns from its excited...

A hydrogen atom is in its third excited state. The atom emits a
1.88E+3nm wavelength photon. Determine the maximum possible orbital
angular momentum of the electron after emission. Express your
answer as multiples of hbar.

A. Determine the wavelength of the light absorbed when an
electron in a hydrogen atom makes a transition from an orbital in
which n=2 to an orbital in which n=7. Express the wavelength in
nanometers to three significant figures.
B. An electron in the n=6 level of the hydrogen atom relaxes to
a lower energy level, emitting light of λ=93.8nm. Find the
principal level to which the electron relaxed. Express your answer
as an integer.
Can you explain it in...

Suppose that an electron is in an excited state of a Hydrogen
atom at the n = 4 energy level. (a) How
many different states are available for that electron to
occupy?(b) Suppose that the electron falls
directly to the ground state, causing a single photon to be
released from the atom. What is the photon’s wavelength?
(c) After its release, the photon collides with an
electron at rest, and scatters off at a 60o angle with
respect to its...

Suppose that an electron is in an excited state of a Hydrogen
atom at the n = 4 energy level.
(a) How many different states are available for
that electron to occupy?
(b) Suppose that the
electron falls directly to the ground state, causing a single
photon to be released from the atom. What is the photon’s
wavelength?
(c) After its
release, the photon collides with an electron at rest, and scatters
off at a 60o angle with respect to...

Light is emitted from a hydrogen atom as an electron in the atom
jump from the n=9 orbit to the n=3 orbit.
What is the energy of the emitted photon in eV?
(b) What are the frequency and wavelength of the photon?
(c) In which frequency range (UV, visible, IR) is the emitted
electromagnetic radiation? Justify your answer.

An excited hydrogen atom emits light with a wavelength of 397.2
nm to reach the
energy level for which n = 2. In which principal quantum level did
the electron
begin? (c = 3.00 x 108 m/s, h = 6.63 x 10-34 J•s, RH = 2.18 x
10-18J).

Consider a Hydrogen atom with the electron in the n = 7 shell.
What is the energy of this system? (The magnitude of the ground
state energy of the Hydrogen atom is 13.6 eV.) Tries 0/20 How many
subshells are in this shell? Tries 0/20 How many electron orbits
are in this main shell? Tries 0/20 How many electrons would fit in
this main shell?

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